Dear AP Chemistry Student & Parents,
I look forward to having you as a part of my AP Chemistry class for the 2014-2015 school year. This letter
contains information that pertains to your AP Chemistry Summer assignment. Each of the following must be
completed. AP Chemistry is a fast-paced course that begins with new material in the very first week. This
assignment must be completed so that you do not fall behind at the very beginning of the course.
We will
have a summer assignment quiz on the first day of class.
As difficult as AP Chemistry is, you will find that it will never be easier to learn College Freshmanlevel Chemistry than it is now! There are several reasons for this:
a) High school classes are generally smaller than college classes. It is not unusual for freshman college
classes to have 200 or more students! In this situation, it is nearly impossible to ask a question during class or
get any individual attention after class. In AP Chemistry, we always take time for questions and answers.
b) Most college professors don't regard teaching Freshman Chemistry as a priority for their job –
many concentrate on their research, and consider teaching to be an interruption and distraction to that end.
At our school, teaching is our Number 1 priority and we do it well!
c) At times Freshman Chemistry is used to "weed out" students. Most colleges prefer not to have
large class sizes in their upper division courses. Therefore the grades and difficulty level of the freshman
courses are adjusted so that only small numbers of very outstanding students will be able to move on. This
can result in a large portion of students in freshman chemistry flunking the course! At our school we don't
have these kinds of pressures, and all students are encouraged to become successful.
d) AP Chemistry will teach you to think at higher levels. In AP Chemistry, you will be forced to think
and apply concepts to new situations, and even derive your own theories from application. This is excellent
preparation for the higher levels of thinking required in college.
The summer assignment is mainly a review of first year Chemistry. The quiz will encourage you to do most of
the memorization for the course before the school year begins. This early work will allow us to spend more
time later on more difficult topics. You will find the summer assignment and the review for the "first day quiz" at
the end of this letter.
I will say that there is fun to be had in this course, as well as the satisfaction of challenging yourself to the
limit of your academic ability. In the past we have had class field trips and parties to celebrate our successes.
1. Memorize Formulas, Charges, and Names for all of the Ions given on the handout. The list includes both
the polyatomic and monatomic ions. Make sure that you know names and formulas. Also, for the
monatomic ions make sure you know both the stock and classical names. You must know how to write
correct chemical formulas using these ions.
2. Memorize Solubility Rules for the Soluble and Insoluble Ionic Compounds. You need to be able to look
at the formula for a compound and know if that compound will be soluble or insoluble in a solution.
3. Memorize Formulas and Names for the Common Acids and Compounds:
a.
Hydrochloric Acid – HCl
s.
Ca(OH)2 slaked lime (lime water)
b.
Sulfuric Acid – H2SO4
c.
Phosphoric Acid – H3PO4
t.
CaSO4 gypsum, plaster of paris
d.
Acetic Acid – HC2H3O2
u.
Fe3O4 or Fe2O3 rust
e.
Carbonic Acid – H2CO3
v.
HCHO formaldehyde
f.
Nitric Acid – HNO3
g.
AlK(SO4)2·12H2O alum
h.
CH4 methane
i.
C6H6 benzene
j.
C10H8 naphthalene (mothballs)
k.
CHCl3 chloroform
l.
CH3OH methyl alcohol or methanol
(wood alcohol)
m. C2H5OH ethyl alcohol or ethanol
(drinking alcohol)
n.
CH3COCH3 acetone
o.
C3H5(OH)3 glycerin
p.
C6H8O6 L-ascorbic acid (vitamin C)
q.
CaCO3 chalk, marble, limestone
r.
CaO quicklime
w. H2O water
x.
Hg quicksilver
y.
K2CO3 potash
z.
MgO magnesia
aa. MgSO4 epsom salts
bb. NH3 ammonia
cc. N2O laughing gas
dd. Na2CO3 soda ash
ee. NaCl table salt
ff. NaHCO3 baking soda
gg. NaNO3 saltpeter
hh. NaOCl bleach
ii.
NaOH caustic soda or lye
jj.
SiO2 sand, quartz
4. Review basic chemistry concepts while completing the AP Chemistry Summer Assignment Worksheet
to make sure that you are ready for the quiz on our first day.
You will have a quiz on the first day of class when you return from break. Please do not put this assignment off
until the last minute. You will not be able to get it done. A failing grade on this test will tell me that you are not
ready to do the work necessary in AP Chemistry and you will be asked to attend tutoring for the first two
weeks of the semester. Please do not hesitate to contact me if you have any questions. I can be reached by email. Thank you in advance for your cooperation and hard work. I look forward to having you in class! It will be
a blast…sometimes quite literally!
Sincerely,
Mr. Youngberg (AKA-Mr. Y)
Email: threegorgesdam@comcast.net Please type “AP Chemistry” your email title.
Chemistry Study Sheet: Ions and Ionic Substances
Cations
Strontium Sr 2
Fluoride F 1
Tin (II) Sn 2 (IV) Sn 4
Hydroxide OH 1
Ammonium NH 41
Zinc Zn 2
Hypochlorite ClO 1
Antimony (III) Sb 3 (V) Sb 5
Anions
Iodide I
Arsenic (III) As 3 (V) As 5
Acetate C2H 3O21
Monohydrogen phosphate HPO42
Barium Ba 2
Arsenate AsO43
Nitride N
Bicarbonate(carbonic acid) HCO31
Nitrate NO31
Calcium Ca 2
Binoxalate HC2O41
Nitrite NO21
Cadmium Cd 2
Bisulfate (sulfuric acid) HSO 41
Oxalate C 2O 42
Chromium (II) Cr 2 (III) Cr 3
Bisulfide(Hydrosulfuric acid) HS 1
Oxide O 2
Cobalt (II) Co 2 (III) Co 3
Bisulfite(sulfurous acid) HSO31
Perchlorate ClO41
Copper (I) Cu 1 (II) Cu 2
Borate BO33
Permanganate MnO 41
3
Aluminum Al
3
Bismuth (III) Bi (V) Bi
Hydrogen H
5
1
Bromide Br
1
1
3
Peroxide O22
Iron (II) Fe 2 (III) Fe 3
Carbonate CO32
Phosphate PO 43
Lead (II) Pb 2 (IV) Pb 4
Chlorate ClO31
Phosphide P
Chloride Cl 1
Silicate SiO32-
Chlorite ClO21
Sulfate SO42
Chromate CrO 42
Sulfide S 2
Cyanide CN 1
Sulfite SO32
Dichromate Cr2O72
Thiocyanate SCN 1
Lithium Li
1
Magnesium Mg
2
2
Manganese (II) Mn (IV) Mn
1
Mercury (I) Hg (II) Hg
Nickel (II) Ni
2
Potassium K
1
Silver Ag
1
Sodium Na 1
(III) Ni
3
2
4
Dihydrogen phosphate H 2PO41
Ferrocyanide Fe (CN )64
Ferricyanide Fe (CN )63
3
Solubility Rules
Rule
1
Ion(s)
Cl-,
Br-
Rule
,
I-
Exceptions
Most chlorides, bromides, and
AgCl, AgBr, AgI, Hg2Cl2,
iodides are soluble.
Hg2Br2, Hg2I2, PbCl2,
PbBr2, PbI2 (silver, mercury
and lead)
2
F-
Most fluorides are soluble
MgF2, CaF2, SrF2, BaF2,
PbF2
(magnesium, lead, calcium,
strontium, and barium)
3
SO4
2-
Most sulfates are soluble
CaSO4, SrSO4,
BaSO4, Ag2SO4,
Hg2SO4, and PbSO4
(silver, mercury and lead,
calcium, strontium, and
barium)
4
CO32-
Most carbonates are insoluble
Group 1A and ammonium
carbonates
5
PO43-
Most phosphates are insoluble
Group 1A and ammonium
phosphates
6
S2-
Most sulfides are insoluble
Group 1A and ammonium
sulfides
7
OH-
Most hydroxides are insoluble
Group 1A hydroxides and
Ca(OH)2, Sr(OH)2, and
Ba(OH)2
(calcium, strontium, barium)
8
Li+, Na+,
Group 1A and ammonium
K+, NH4+
compounds are soluble
None
(Alkali metals and ammonium)
9
C2H3O2,
Acetates, nitrates, chlorates, and None
NO3-,
perchlorates are soluble
ClO3-,
ClO4-
AP Chemistry Summer Assignment
The following assignment is to be completed and brought on the first day of class.
Nomenclature
Name these binary compounds of two nonmetals.
1.
IF7
4.
N2O4
7.
PCl3
2.
N2O5
5.
As4O10
8.
S2Cl2
3.
XeF2
6.
SF6
Name these binary compounds with a fixed charge metal.
9.
AlCl3
12. KI
15. CaF2
10. MgO
13. SrBr2
16. Al2O3
11. BaI2
14. Na2S
Name these binary compounds of cations with variable charge.
17. CuCl2
20. PbCl4
23. AuI3
18. Fe2O3
21. Cu2S
24. CoP
19. SnO
22. HgS
Name these compounds with polyatomic ions.
25. Fe(NO3)3
28. Ca(ClO3)2
31. NH4NO2
26. NaOH
29. KNO2
32. Cu2Cr2O7
27. Cu2SO4
30. NaHCO3
Name these binary acids
33. HCl
34. HI
Name these acids with polyatomic ions.
35. HClO4
38. H3PO4
41. H2C2O4
36. H2SO4
39. HNO2
42. H2CO3
37. HC2H3O2
40. H2CrO4
Name these compounds appropriately.
43. CO
48. OF2
53. CuCr2O7
44. NH4CN
49. LiMnO4
54. K2O
45. HIO3
50. HClO
55. FeF3
46. NI3
51. HF
56. KC2H3O2
47. AlP
52. SO2
57. MnS
58. Tin (IV) phosphide
62. Sulfurous acid
66. Gallium arsenide
59. Copper (II) cyanide
63. Lithium silicate
67. Cobalt (II) chromate
60. Magnesium hydroxide
64. Potassium nitride
68. Zinc fluoride
61. Sodium peroxide
65. Chromium (III) carbonate
69. Dichromic acid
Write the formulas.
Solubility rules
Review solubility rules and identify each of the following compounds as soluble or insoluble in water.
70. Na2CO3
75. (NH4)2S
80. PbCl2
71. CoCO3
76. AgI
81. CuSO4
72. Pb(NO3)2
77. Ni(NO3)2
82. Li2O
73. K2S
78. KI
83. Mn(C2H3O2)2
74. BaSO4
79. FeS
84. Cr(OH)3
85. AgClO3
86. Sn(SO3)4
87. FeF2
Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the
products. If yes, identify the precipitate.
88. silver nitrate and potassium chloride
89. magnesium nitrate and sodium carbonate
90. strontium bromide and potassium sulfate
91. cobalt (III) bromide and potassium sulfide
92. ammonium hydroxide and copper (II) acetate
93. lithium chlorate and chromium (III) fluoride
Balancing Equations
Balance the following equations with the lowest whole number coefficients.
94. S8 +
O2  SO3
95. C10H16 + Cl2 
96. Fe +
O2 
C +
98. KClO3 
HCl
Fe2O3
97. C7H6O2 + O2  CO2 + H2O
99. H3AsO4 
KCl + O2
As2O5 + H2O
100. V2O5 + HCl  VOCl3 +
H2O
101. Hg(OH)2 + H3PO4  Hg3(PO4)2 + H2O
Stoichiometry and Limiting Factor
102. Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide?
Na2O + H2O  2NaOH
103. What mass of sodium choride is formed along with 45.0g of oxygen gas?
2NaClO3  2NaCl + 3O2
104. What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen?
4NH3 + 5O2  4NO + 6 H2O
105. If the reaction in #104 is done with 25.0g of each reactant, which would be the limiting factor?
106. Na2S + 2AgNO3  Ag2S + 2NaNO3
a. If the above reaction is carried out with 50.0g of sodium sulfide and 35.0g of silver nitrate, which is the limiting factor?
b. What mass of the excess reactant remains?
c. What mass of silver sulfide would precipitate?
107. What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium hydroxide with 50.0g of
aluminum?
6NaOH + 2Al  2Na3AlO3 + 3H2